Unit 9: Gas Laws Quiz

Match the following Laws to their definitions

• Charles' Law

• The total pressure is equal to the sum of all of the partial pressures.

• Dalton's Law of Partial Pressures

• If pressure increases, then temperature increases.

• Gay-Lussac's Law

• If volume increases, then the number of particles increases

• Avogadro's Law

• If pressure increases, then volume decreases.

• Boyle's Law

• If volume increases, then temperature increases.

How many moles of gas occupy 98 L at a pressure of 2.8 atm and a temperature of 292 K?

• 11 mol

• 22 mol

• 0.56 mol

• 2.56 mol

In a balloon, there is 0.23 atm of O₂, 0.5 atm of N₂, and 1.2 atm of CO₂. What is the total pressure inside the balloon?

• 1.93 atm

• 1.93 torr

• 0.173 atm

• 0.173 torr

A balloon is filled with 35 L of helium in the morning when the temperature is 20^oC. By noon, the temperature has risen to 45^oC. What is the new volume of the balloon?

• 38 L

• 15.6 L

• 32 L

• 27.8 L

Tags

NGSS.HS-PS3-4

CaCO₃ decomposes at 1200^oC to form CO₂ gas and CaO. If 25 L of CO₂ are collected at 1200^OC, what will the volume of this gas be after it cools to 25^oC?

• 5.1 L

• 10.2 L

• 1200 L

• 124 L

A helium balloon with an internal pressure of 1 atm and a volume of 4.5 L at 20^oC is released. What volume will the balloon occupy at an altitude where the pressure is 0.6 atm and the temperature is -20^oC?

• 6.48 L

• 13.6 L

• 7.5 L

• 2.91 L

A 75 L container holds 62 moles of gas at a temperature of 215^o C. What is the pressure in atmospheres inside the container?

• 33 atm

• 21 atm

• 15 atm

• 42 atm

6.0 L of gas in a piston at a pressure of 1.0 atm are compressed until the volume is 3.5 L. What is the new pressure inside the piston?

• 1.7 atm

• 2.2 atm

• 0.58 atm

• 0.82 atm

The initial volume of a gas at a pressure of 3.2 atm is 2.9 L. What will the volume be if the pressure is increased to 4.0 atm?

• 2.3 L

• 2.3 mL

• 2.3 atm

• 2.3 K

The gases in a hair spray can are at a temperature of 27^oC and a pressure of 3.2 atm. If the gases in the can reach a pressure of 9.8 atm, the can will explode. To what temperature must the gases be raised in order for the can to explode?

• 919 K

• 98 K

• 83 K

• 8.8 K